4 years ago

What is the balenced formula for C3H8+O2

Chemistry

1 answer:

balandron [24]4 years ago

4 0

C3H8 + 5O2 -----> 3CO2 + 4H2O

This is propane burning in air or pure oxygen.

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How many kilojoules of heat are required to vaporize 50.0 g of ethanol (MM = 46.07 g). Its molar heat of vaporization is 43.5 kJ

guajiro [1.7K]

Answer:

ΔH = 41.7 kj

Given data:

Mass of ethanol = 50 g

Heat required to vaporize = ?

Boiling point of ethanol = 78.3°C

Molar heat of vaporization = 38.6 kj/mol

Solution:

First of all we will calculate the number of moles.

Number of moles = mass / molar mass

Number of moles = 50 g/ 46.07 g/mol

Number of moles = 1.08 mol

ΔH = 38.6 kj/mol ×1.08 mol

ΔH = 41.7 kj

Explanation:

8 0

4 years ago

You want to make 500 ml of a 1 N solution of sulfuric acid (H2SO4, MW: 98.1). How many grams of sulfuric acid do you need?

umka21 [38]

Answer:

24.525 g of sulfuric acid.

Explanation:

Hello,

Normality (units of eq/L) is defined as:

$N=\frac{eq_{solute}}{V_{solution}}$

Since the sulfuric acid is the solute, and we already have the volume of the solution (500 mL) but we need it in liters (0.5 L, just divide into 1000), the equivalent grams of solute are given by:

$eq_{solute}=N*V_{solution}=1\frac{eq}{L}*0.5L=0.5 eq$

Now, since the sulfuric acid is diprotic (2 hydrogen atoms in its formula) 1 mole of sulfuric acid has 2 equivalent grams of sulfuric acid, so the mole-mass relationship is developed to find its required mass as follows:

$m_{H_2SO_4}=0.5eqH_2SO_4(\frac{1molH_2SO_4}{2 eqH_2SO_4}) (\frac{98.1 g H_2SO_4}{1 mol H_2SO_4} )\\m_{H_2SO_4}=24.525 g H_2SO_4$