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Mekhanik [1.2K]

3 years ago

7

When 0.2mol of calcium reacts with 880g of water 2.24L of hydrogen gas form at STP How would the amount of hydrogen produced cha

nge if the volume of water was decreased to 440mL 400g?

1 answer:

Mila [183]3 years ago

4 0

It would half, you have half the amount of reactant and so you would only produce 1.12 litres of hydrogen

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Lera25 [3.4K]

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6 0

3 years ago

Read 2 more answers

What is one thing that all polysaccharides have in common?

VashaNatasha [74]

<h3><u>Answer</u>;</h3>

D. All polysaccharides are made up of carbon, hydrogen, and oxygen.

<h3><u>Explanation</u>;</h3>

A polysaccharide is a large molecule made of many monomers called monosaccharides such as glucose, galactose, fructose, etc.
Polysaccharides can be homopolysaccharides, where all monosaccharides are the same or heteropolysaccharide in which the monosaccharides vary.
They may be linear, where a molecule of polysaccharides has straight chain of monosaccharides, or branched polysaccharides in which a chain has arms.
<em><u>All polysaccharides contain oxygen, hydrogen and carbon atoms like all the carbohydrates.</u></em>

4 0

3 years ago

Steam reforming of methane ( CH4 ) produces "synthesis gas," a mixture of carbon monoxide gas and hydrogen gas, which is the sta

Hatshy [7]

<u>Answer:</u> The pressure equilibrium constant for the reaction is 1473.8

<u>Explanation:</u>

We are given:

Initial partial pressure of methane gas = 2.4 atm

Initial partial pressure of water vapor = 3.9 atm

Equilibrium partial pressure of hydrogen gas = 6.5 atm

The chemical equation for the reaction of methane gas and water vapor follows:

$CH_4+H_2O\rightleftharpoons CO+3H_2$

<u>Initial:</u> 2.4 3.9

<u>At eqllm:</u> 2.4-x 3.9-x x 3x

Evaluating the value of 'x':

$\Rightarrow 3x=6.5\\\\x=2.167$

So, equilibrium partial pressure of methane gas = (2.4 - x) = [2.4 - 2.167] = 0.233 atm

Equilibrium partial pressure of water vapor = (3.9 - x) = [3.9 - 2.167] = 1.733 atm

Equilibrium partial pressure of carbon monoxide gas = x = 2.167 atm

The expression of $K_p$ for above equation follows:

$K_p=\frac{p_{CO}\times (p_{H_2})^3}{p_{CH_4}\times p_{H_2O}}$

Putting values in above equation, we get:

$K_p=\frac{2.167\times (6.5)^3}{0.233\times 1.733}\\\\K_p=1473.8$

Hence, the pressure equilibrium constant for the reaction is 1473.8

5 0

4 years ago

Find the molarity of a solution in which 0.99 mol of NaCl are dissolved in 2.5 L of solution.

rusak2 [61]

Answer:

0.369M

Explanation:

$\boxed{Molarity = mole \div volume}$

☆ Volume has to be in litres

Molarity of solution

= 0.99 ÷2.5

= 0.369 M

3 0

3 years ago

Correctly balance this equation: <br> K+O2=K2O

jeka57 [31]

K + 02 ---> K20

4K + O2 ---> 2K2O

7 0

3 years ago