During the analysis, 0.163 g h2o and 0.600 g co2 are produced. calculate the amount (mol) h2o formed by combustion of 0.400 g vitamin c

Here we have to get the moles of water generated by the combustion of vitamin C.

4 moles of water (H₂O) will generate from the combustion of vitamin C.

The vitamin C is the ascorbic acid having the molecular formula C₆H₈O₆. On decomposition it produces water (H₂O) and carbon di oxide (CO₂).

The molecular weight of ascorbic acid is 176.12 g/mole.

In this analysis 0.163g of H₂O produces from 0.400g of vitamin C.

Thus from 176.12 g of vitamin C ×176.12 = 71.768 g of H₂O will produce.

The molecular weight of H₂O is 18 g/mole. Thus 71.768 g is equivalent to = 3.98 ≅ 4

Thus 1 mole of vitamin C (ascorbic acid) produces 4 moles of water on combustion.

The balanced combustion [in presence of excess oxygen (O₂)] reaction can be written as- C₆H₈O₆ + 5O₂ = 4H₂O + 6CO₂.

Thus the moles of water generated from combustion of vitamin C is determined.

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

plasma is the state of matter where the substance is ionized and has no definite shape or volume. the fact of being ionized makes the substance a good electrical conductor.