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3 years ago

In the reaction :N2 + 3H2----2NH3 how many grams of H2 are needed to produce 1 mole on ammonia

1 answer:

3 0

Start with moles of ammonia you want to produce, then convert to how many moles of H2 you need to get one mole of ammonia, then convert that to grams :)

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A 257-ml sample of a sugar solution containing 1.10 g of the sugar has an osmotic pressure of 31.5 mm hg at 39°c. what is the mo

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3 years ago

What amount of heat is required to raise the temperature of 20 grams of water from 10°C to 30°C? The specific heat of water is 4

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Q=MCdeltaT
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3 years ago

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A 0.2500 g sample of an alloy reacts with to form hydrogen gas: 2Al(s) + 6H+(aq) 2Al3+(aq) + 3H2(g) Zn(s) + 2H+(aq) Zn2+(aq) + H

fenix001 [56]

Answer: The mass percent of zinc in the alloy is 78.68 %

Explanation:

We are given:

Mass of sample of alloy = 0.2500 g

Let the mass of aluminium be 'x' grams and mass of zinc will be (0.2500 - x) g

To calculate the amount of hydrogen gas produced, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 755 mmHg

V = Volume of the gas = 0.147 L

T = Temperature of the gas = $25^oC=[25+273]K=298K$

R = Gas constant = $62.3637\text{ L.mmHg }mol^{-1}K^{-1}$

n = number of moles of hydrogen gas = ?

Putting values in above equation, we get:

$755mmHg\times 0.147L=n\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 298K\\\\n=\frac{755\times 0.147}{62.3637\times 298}=0.00597mol$

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For Aluminium:

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

$\text{Moles of aluminium}=\frac{x}{27}mol$

The chemical equation follows:

$2Al(s)+6H^+(aq.)\rightarrow 2Al^{3+}(aq.)+3H_2(g)$

By Stoichiometry of the reaction:

2 moles of aluminium produces 3 moles of hydrogen gas

So, $\frac{x}{27}$ moles of aluminium will produce = $\frac{3}{2}\times \frac{x}{27}=\frac{3x}{54}mol$ of hydrogen gas

For Zinc:

Molar mass of zinc = 65.4 g/mol

Putting values in equation 1, we get:

$\text{Moles of zinc}=\frac{(0.25-x)}{65.4}mol$

The chemical equation follows:

$Zn(s)+2H^+(aq.)\rightarrow Zn^{2+}(aq.)+H_2(g)$

By Stoichiometry of the reaction:

1 mole of zinc produces 1 moles of hydrogen gas

So, $\frac{(0.25-x)}{65.4}$ moles of zinc will produce = $\frac{1}{1}\times \frac{(0.25-x)}{65.4}=\frac{(0.25-x)}{65.4}mol$ of hydrogen gas

Equating the moles of hydrogen gas:

$\Rightarrow 0.00597=\frac{3x}{54}+\frac{(0.25-x)}{65.4}\\\\x=0.0533g$

To calculate the mass percentage of zinc in alloy, we use the equation:

$\text{Mass percent of zinc}=\frac{\text{Mass of zinc}}{\text{Mass of alloy}}\times 100$

Mass of zinc = (0.2500 - x) = [0.2500 - 0.0533] = 0.1967 g

Mass of alloy = 0.2500 g

Putting values in above equation, we get:

$\text{Mass percent of zinc in alloy}=\frac{0.1967g}{0.2500g}\times 100=78.68\%$

Hence, the mass percent of zinc in the alloy is 78.68 %

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4 years ago

7. How many electrons can be held in the energy level n = 4?

Dahasolnce [82]

Answer:

32 electrons

Explanation:

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3 years ago

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