Help me now, please! _SnO2 + _H2 + Energy → _Sn + _H2O

1) Find the correct coefficients for all the "_"s.
2) Answer this question: If there is enough energy and H2, then how many moles of Sn02 will react with 2 moles of H2 and produce 1 mole of Sn and 2 moles of H2O? How many moles of SnO2 does this balanced equation represent?

1. SnO2 = 1; H2 = 2; Sn = 1; H2O = 2

2. I mole of SnO2 is required to react with 2 moles of H2 to produce 1 mole of Sn and 2 moles of H20.

The balanced equation represents 1 mole of SnO2

3. Total mass of reactants and products are each 154.71g respectively

Explanation:

1. According to the law of conservation of mass, the total mass of reactants in a chemical reaction is equal to the mass of products.

Therefore, a balanced chemical equation has equal number of moles of each atom on the reactants side and on the product side. The balanced chemical equation for the reaction above will be:

Sn02 + 2H2 + Energy > Sn + 2H2O

Sn has 1 mole of atoms on both sides

O has 2 moles of atoms on both sides

H has 4 miles of atoms on both sides.

2. According to the balanced chemical equation above,

1 mole of SnO2 reacts with 2 moles of H2 to produce 1 mole of An and 2 moles of H20.

This balanced equation represents 1 mole of SnO2.

3. The atomic masses of Sn, O and H are 118.71g, 16g and 1g respectively.

Therefore, the molar masses of the reactants and products are;

SnO2 = 118.71 + 16 * 2 = 150.72g

H2 = 2 *1 = 2g

H2O = 2 * 1 + 16 = 18g

Total mass of reactants = 150.71g + 2 * 2g = 154.72g

Total mass of products = 118.71 + 2 * 18g = 154.71g

consider the reaction below.

 no rx

at 500 k, the reaction is at equilibrium with the following concentrations.

[pci5]= 0.0095 m

[pci3] = 0.020

[ci2] = 0.020 m

what is the equilibrium constant for the given reaction?

0.042

0.42

2.4

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