The combustion reaction of acetylene gas is represented by this equation:

2 C2H2(g) + 5 O2(g) ==> 4 CO2(g) + 2 H2O(g)

How many grams of CO2 and grams of H2O are produced when 52.0g C2H2 burns in oxygen?

Convert 52.0 g C2H2 to moles. moles = grams/molar mass.

Using the coefficients in the balanced equation, convert moles acetylene to moles CO2 and do the same thing for moles H2O.

Now convert those moles to grams. g = moles x molar mass.

When 1 mole of tin IV oxide is heated with 2 moles of hydrogen gas, 1 mole of tin metal and 2 moles of water vapor are generated.

SnO¿ + 2H¿d Sn + 2H¿O
How many moles of tin metal will be produced when 0.74 moles of tin IV oxide is heated?

The answer would be 0.74 I just answered this question and got the go

To find the number of grams of CO2 and H2O produced when 52.0 g of C2H2 burns in oxygen, we need to use stoichiometry. Stoichiometry is a concept that allows us to relate the amounts of reactants and products in a chemical reaction.

First, we need to determine the molar masses of the substances involved in the reaction. The molar mass of C2H2 is 26.04 g/mol (2 * 12.01 + 2 * 1.01), O2 is 32.00 g/mol (2 * 16.00), CO2 is 44.01 g/mol (12.01 + 2 * 16.00), and H2O is 18.02 g/mol (2 * 1.01 + 16.00).

Next, we'll convert the given mass of C2H2 into moles. We can do this by dividing the mass by the molar mass:
52.0 g / 26.04 g/mol = 1.995 mol C2H2 (rounded to three decimal places).

Now, using the balanced equation, we can determine the moles of CO2 and H2O produced from the moles of C2H2.

From the equation, we can see that 2 moles of C2H2 react to produce 4 moles of CO2 and 2 moles of H2O.

So, using the ratio derived from the equation, we can calculate the moles of CO2 produced:
1.995 mol C2H2 * (4 mol CO2 / 2 mol C2H2) = 3.99 mol CO2 (rounded to two decimal places).

Similarly, we can calculate the moles of H2O produced:
1.995 mol C2H2 * (2 mol H2O / 2 mol C2H2) = 1.995 mol H2O.

Finally, we can convert the moles of CO2 and H2O to grams by multiplying them by their respective molar masses.

Grams of CO2 produced:
3.99 mol CO2 * 44.01 g/mol = 175.95 g CO2 (rounded to two decimal places).

Grams of H2O produced:
1.995 mol H2O * 18.02 g/mol = 35.89 g H2O (rounded to two decimal places).

Therefore, when 52.0 g of C2H2 burns in oxygen, approximately 175.95 g of CO2 and 35.89 g of H2O are produced.