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Anvisha [2.4K]
2 years ago
12

Calcium is a metal.

Chemistry
1 answer:
kirza4 [7]2 years ago
3 0

Answer:

22.22 g

Explanation:

The balanced reaction equation is;

Ca(s) + 2HCl(aq) → CaCl2(aq) + H2(g)

Number of moles of calcium reacted = 8.02g/40.1g/mol = 0.2 moles of Calcium

From the reaction equation;

1 mole of Ca yields 1 mole of CaCl2

Hence 0.2 moles of Ca also yields 0.2 moles of CaCl2

Mass of calcium chloride produced = number of moles * molar mass

Mass of calcium chloride = 0.2 moles of CaCl2 * 111.1g/mol = 22.22 g

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You are growing a garden and notice that the soil is always wet. What type of soil do you have?
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Are all atoms of the same element identical? Back up your answer with evidence and examples. pls help
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The chemical reaction for the formation of syngas is: CH4 + H2O -> CO + 3 H2 What is the rate for the formation of hydrogen,
grin007 [14]

Answer :  The rate for the formation of hydrogen is, 1.05 M/s

Explanation :

The general rate of reaction is,

aA+bB\rightarrow cC+dD

Rate of reaction : It is defined as the change in the concentration of any one of the reactants or products per unit time.

The expression for rate of reaction will be :

\text{Rate of disappearance of A}=-\frac{1}{a}\frac{d[A]}{dt}

\text{Rate of disappearance of B}=-\frac{1}{b}\frac{d[B]}{dt}

\text{Rate of formation of C}=+\frac{1}{c}\frac{d[C]}{dt}

\text{Rate of formation of D}=+\frac{1}{d}\frac{d[D]}{dt}

Rate=-\frac{1}{a}\frac{d[A]}{dt}=-\frac{1}{b}\frac{d[B]}{dt}=+\frac{1}{c}\frac{d[C]}{dt}=+\frac{1}{d}\frac{d[D]}{dt}

From this we conclude that,

In the rate of reaction, A and B are the reactants and C and D are the products.

a, b, c and d are the stoichiometric coefficient of A, B, C and D respectively.

The negative sign along with the reactant terms is used simply to show that the concentration of the reactant is decreasing and positive sign along with the product terms is used simply to show that the concentration of the product is increasing.

The given rate of reaction is,

CH_4+H_2O\rightarrow CO+3H_2

The expression for rate of reaction :

\text{Rate of disappearance of }CH_4=-\frac{d[CH_4]}{dt}

\text{Rate of disappearance of }H_2O=-\frac{d[H_2O]}{dt}

\text{Rate of formation of }CO=+\frac{d[CO]}{dt}

\text{Rate of formation of }H_2=+\frac{1}{3}\frac{d[H_2]}{dt}

The rate of reaction expression is:

\text{Rate of reaction}=-\frac{d[CH_4]}{dt}=-\frac{d[H_2O]}{dt}=+\frac{d[CO]}{dt}=+\frac{1}{3}\frac{d[H_2]}{dt}

As we are given that:

+\frac{d[CO]}{dt}=0.35M/s

Now we to determine the rate for the formation of hydrogen.

+\frac{1}{3}\frac{d[H_2]}{dt}=+\frac{d[CO]}{dt}

+\frac{1}{3}\frac{d[H_2]}{dt}=0.35M/s

\frac{d[H_2]}{dt}=3\times 0.35M/s

\frac{d[H_2]}{dt}=1.05M/s

Thus, the rate for the formation of hydrogen is, 1.05 M/s

6 0
3 years ago
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