When heat is applied to 80 grams of CaCO3, it yields 39 grams of CO2. Determine the percentage of the yield.

The percentage yield of is 90.26%.

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass. The equation used is:

......(1)

Given mass of = 80 g

Molar mass of = 100 g/mol

Plugging values in equation 1:

For the given chemical equation:

By the stoichiometry of the reaction:

If 1 mole of produces 1 mole of

So, 0.8 moles of will produce = of

Molar mass of = 44 g/mol

Plugging values in equation 1:

The percent yield of a reaction is calculated by using an equation:

......(2)

Given values:

Actual value of = 35.2 g

Theoretical value of = 39 g

Plugging values in equation 2:

Hence, the percentage yield of is 90.26%.

yes yes yes yes yes yes yes yes yes yes yes yes yes yes yes

explanation:

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol