Which two types of energy are formed by the transformation shown in the
photo?
A. Chemical energy →
thermal energy
n BiThermal energy
electrical energy
C. Thermal energy – chemical energy
D. Chemical energy - electromagnetic energy
SUBMIT

Answer:

Iron is natural. Paper is man-made

Explanation:

Answer:

iron

Explanation:

Answer:

The predator-prey relationship helps to hold the populations of the two species in equilibrium. ... If the population of prey increases, there is more food for predators. So after a slight period, the predator population is also increasing. If the number of predators increases, more prey is captured.

Explanation:

Answer:

i eat you, you die

Explanation:

thats how life works

Answer:

1. pH = 1.23.

2. [tex]H_2C_2O_4(aq) +OH^-(aq)\rightarrow HC_2O_4^-(aq)+H_2O(l)[/tex]

Explanation:

Hello!

1. In this case, for the ionization of H2C2O4, we can write:

[tex]H_2C_2O_4\rightleftharpoons HC_2O_4^-+H^+[/tex]

It means, that if it is forming a buffer solution with its conjugate base in the form of KHC2O4, we can compute the pH based on the Henderson-Hasselbach equation:

[tex]pH=pKa+log(\frac{[base]}{[acid]} )[/tex]

Whereas the pKa is:

[tex]pKa=-log(Ka)=-log(5.90x10^{-2})=1.23[/tex]

The concentration of the base is 0.347 M and the concentration of the acid is 0.347 M as well, as seen on the statement; thus, the pH is:

[tex]pH=1.23+log(\frac{0.347M}{0.347M} )\\\\pH=1.23+0\\\\pH=1.23[/tex]

2. Now, since the addition of KOH directly consumes 0.070 moles of acid, we can compute the remaining moles as follows:

[tex]n_{acid}=0.347mol/L*1.00L=0.347mol\\\\n_{acid}^{remaining}=0.347mol-0.070mol=0.277mol[/tex]

It means that the acid remains in excess yet more base is yielded due to the effect of the OH ions provided by the KOH; therefore, the undergone chemical reaction is:

[tex]H_2C_2O_4(aq) +OH^-(aq)\rightarrow HC_2O_4^-(aq)+H_2O(l)[/tex]

Which is also shown in net ionic notation.

Best regards!

Answer:

0.548 moles of HBr are required

Explanation:

Given data:

Number of moles of  hydrobromic acid = ?

Moles of bromine formed = 0.274 mol

Solution:

Chemical equation:

2HBr     →   H₂  + Br₂

Now we will compare the moles of HBr with Br₂.

               Br₂           :           HBr

               1               :            2

               0.274       :           2×0.274=0.548

Thus, 0.548 moles of HBr are required.

Answer:

true

Explanation:

Answer:

Molecular movement

Explanation:

When an object gets hotter, its molecules gain more kinetic energy and then move faster. Therefore, the fast-moving molecules will cause those around them to move faster as well, and the colder (or more slow-moving molecule object) object or part is heated up.

PLS GIVE BRAINLIEST

Answer:

76.4oC or 169.52oF

Explanation:

That's the amount of heat needed

The heat capacity is the heat amount lost or gained by the object in a thermodynamic system. The heat needed to raise the temperature of the water is 1117.7 Joules.

Heat capacity (q) is the heat an object loses or gains to alter the temperature of the thermodynamic system by a difference of a degree Celsius. The heat capacity is given by the mass, specific heat capacity, and temperature change.

Given,

Mass of water (m) = 3.50 gm

Specific heat (c) = 4.18 J/ g°C

The temperature change (∆T) = T₂ - T₁

= 98.8 °C - 22.4 °C

= 76.4 °C

The heat capacity is given as,

q = mc∆T

Substituting values above:

q = 3.50 gm × 4.18 J/ g °C × 76.4 °C

q = 1117.7 J

Therefore, 3.50 g of water has a heat capacity of 1117.7 Joules.

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Answer:

Explanation:

no of moles=given mass/molar mass

no of moles=150 g/207.19

no of moles=0.72

We will use dimensional analysis to answer this question.

[tex]150 g * \frac{1 g}{207.19 mol} = 0.724 mol[/tex]

The answer is 0.724 mol.

Answer:

1.Reaction rate is how fast a chemical reaction proceeds.

2.Nature of the reaction, Pressure factor

, Solvent, Catalyst and inhibitors.

3.Physical change is a temporary change. A chemical change is a permanent change. A Physical change affects only physical properties i.e. shape, size, etc.

4. One example of the effect of temperature is the use of lightsticks or glowsticks.

5.When the particle size of a fixed mass of a solid reactant becomes smaller, the total exposed surface area becomes larger, the rate of reaction increases. an example could be ice and water when the atoms are stuck together a solid but all over the place as a liquid.

6. Sometimes a reaction depends on catalysts to do their job. In that case, changing the concentration of the catalyst can speed up or slow down the reaction. For example, enzymes speed up biological reactions, and their concentration affects the rate of reaction.

7.A catalyst is a chemical substance that affects the rate of a chemical reaction by altering the activation energy required for the reaction to proceed. For example, a catalyst could cause a reaction between reactants to happen at a faster rate or at a lower temperature than would be possible without the catalyst.

Explanation:

I hope this helps have a great day! :)

mass = 20.48 g

moles=0.1895

In general, the gas equation can be written  

where  

P = pressure, atm  

V = volume, liter  

n = number of moles  

R = gas constant = 0.08205 L.atm / mol K  

T = temperature, Kelvin  

P=0.23 atm

V=20 L

T=23+273=296 K

[tex]\tt n=\dfrac{PV}{RT}=\dfrac{0.23\times 20}{0.082\times 296}=0.1895[/tex]

mass SF₄ (MW=108,07 g/mol) :

[tex]\tt 0.1895\times 108,07 g/mol=20.48~g[/tex]

Answer:

0.805 M.

Explanation:

Hello!

In this case, since the molarity of a solution is computing by dividing the moles of solute over the volume of solution in liters (M=n/V), for 15.0 g of potassium chloride (74.55 g/mol) we compute the corresponding moles:

[tex]n=15.0gKCl*\frac{1molKCl}{74.55gKCl}=0.201molKCl[/tex]

Next, since the volume is 0.2500 in liters, the molarity turns out:

[tex]M=\frac{0.201mol}{0.2500L} \\\\M=0.805M[/tex]

Best regards!

Answer:

26.982

Explanation:

Use the periodic table

Answer:

When all molecules in a system stop moving completely, there is zero thermal energy

Explanation:

It is impossible to reach though

Answer:

1.5 moles of Fe produced.

Explanation:

Given data:

Moles of FeO react = 1.50 mol

Moles of iron produced = ?

Solution:

Chemical equation:

FeO + CO       →       Fe + CO₂

Now we will compare the moles of ironoxide with iron.

                           FeO          :           Fe

                              1             :             1

                             1.5           :           1.5

Thus from 1.5 moles of FeO 1.5 moles of Fe are produced.                                    

1.5 moles of Fe can be obtained when 1.50 mol of FeO reacts with an excess

of CO

Moles of FeO reacted  = 1.50 mol

Moles of iron produced = ? mol

The chemical equation is given as

FeO + CO       →       Fe + CO₂

Comparisons of FeO and Fe show they are in the ratio 1 : 1

                          FeO          :           Fe

                            1.5           :           1.5

which translates to the number of moles being equal

Therefore, 1.5 moles of FeO 1.5 moles of Fe are produced.    

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Answer:

0 Kelvin is called Absolute Zero. Particles will stop moving, and lose all energy.

Answer:

An example is the formation of ATP, which is an endergonic process and is coupled to the dissipation of a proton gradient.

Explanation:

Hope this helped!

Answer:

carbon-13

Explanation:

Answer:

Explanation:

Answer:

there is your answer hope it helped :3

Answer:

It changes by roughly 1 atm.

Explanation:

Hello!

In this case, since the ideal gas equation differs from the van der Waals' one by the presence of the a and b parameters which correct the assumption of no interactions into the container, they are written as:

[tex]P=\frac{nRT}{V}\\\\P=\frac{RT}{v_m-b}-\frac{a}{v_m^2}[/tex]

Thus, the pressure via the ideal gas equation is:

[tex]P=\frac{0.300mol*0.082\frac{atm*L}{mol*K}*248K}{0.200L}=30.5atm[/tex]

And the pressure via the van der Waals equation, considering the molar volume (vm=0.200L/0.300L=0.667L/mol) is:

[tex]P=\frac{0.082\frac{atm*L}{mol*K}*248K}{0.667L/mol-0.0237L/mol}-\frac{0.0342atm*L^2/mol^2}{(0.667L/mol)^2}\\\\P=31.6atm-0.0769atm\\\\P=31.5atm[/tex]

It means that the pressure change by 1 atm, which is not a significant difference for helium.

The difference in pressure calculated by the two methods is 84 atm.

The ideal gas equation is given by

PV =nRT

From the data given in the question;

P = ?

V = 0.200 L

n =  0.300 mol

T = 248K

R = 0.082 atmLK-1Mol-1

P = nRT/V

P =  0.300 mol × 0.082 atmLK-1Mol-1  × 248K/0.200 L

P = 30.5 atm

From Van der Waals equation;

P = RT/V - b - a/V^2

P =  (0.082 × 248/0.200 - 0.0237)  - (0.0342/ 0.200^2)

P = 114.5 atm

The difference in pressure calculated by the two methods is;

114.5 atm -  30.5 atm = 84 atm

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Answer:

use google

Explanation:

Answer:

it is true bc i looked it up

Answer:

C. The weaker the acid, the higher the pH at the equivalence point.

Explanation:

In a titration, a solution which concentration is known is added gradually to another solution of unknown concentration, until the chemical reaction between the two solutions is complete.

The pH in the equivalence point is equal to 7.00 only if both the acid and base are strong. When one or both reactants are weak, the pH in the equivalence point is not equal to 7.00.

In the equivalence point, the amount of strong base (like NaOH) added is just enough to react stoichiometrically with the weak acid. The resulting solution "only" contains the conjugated base A⁻. A solution of Na⁺A⁻ is the solution of a weak base:

A⁻ + H₂O ⇄ HA + OH⁻              Kb=Kw/Ka

In the equivalence point of the titration of a weak base with a strong base, the pH is higher than 7.00 because at this point the acid is transformed into its conjugate base.

Answer:

[tex]55.2gH_2O[/tex]

Explanation:

Hello!

In this case, since the reaction between hydrogen and oxygen to produce water is:

[tex]2H_2+O_2\rightarrow 2H_2O[/tex]

When equal masses of each reactant go in contact to carry out the reaction, we can identify the maximum mass of yielded water as the fewest mass yielded by each reactant, just as shown below:

[tex]m_{water}^{by\ H_2}=49.0gH_2*\frac{1molH_2}{2.02gH_2}*\frac{2molH_2O}{2molH_2}*\frac{18.02gH_2O}{1molH_2O} =170gH_2O\\\\m_{water}^{by\ O_2}=49.0gO_2*\frac{1molO_2}{32.0gO_2}*\frac{2molH_2O}{1molO_2}*\frac{18.02gH_2O}{1molH_2O} =55.2gH_2O[/tex]

Thus, since hydrogen yields more water than real, we limit the maximum mass of water to those 55.2 g yielded by oxygen as hydrogen would be in excess.

Best regards!

Answer:

1 oxygen and 2 hydrogen

Answer:

3 atm

1.6 g

Explanation:

Step 1: Given data

Step 2: Find partial pressure (P) of CO₂ gas

We will use Henry's law.

C = k × P

P = C / k

P = 0.1 M / 3.3 × 10⁻² M atm⁻¹

P = 3 atm

Step 3: Calculate the mass of CO₂ gas

The molar mass of carbon dioxide is 44.01 g/mol.

0.355 L × 0.1 mol/L × 44.01 g/mol = 1.6 g

Answer: C

Explanation: Everything else is true.