In the equation N2(g) + 3H2(g)--- 2NH3(g), how many liters of hydrogen

2 answers:

5 0

15 L

Explanation:
The important thing to remember about reactions that involve gases kept under the same conditions for pressure and temperature is that the mole ratios that exist between the gases are equivalent to volume ratios.

Delicious77 [7]3 years ago

3 0

Answer:

30 L H2

Explanation:

10 L N2 x <u>3 L H2</u> = 30 L H2

. 1 L N2

Try to verify my answer, Stoichiometry is not easy for me.

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Rust forms when the iron is exposed to water and oxygen.<br> True<br> False

Montano1993 [528]

True

explanation:

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8 0

3 years ago

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11. Calculate the energy required to produce 12.00 mol of CI207 on the basis of the

Ber [7]

Answer: 780 kcal are required to produce 12.00 mol of $Cl_2O_7$

Explanation:

Endothermic reactions are defined as the reactions in which energy of the product is greater than the energy of the reactants. The total energy is absorbed in the form of heat and written along with reactants.

The balanced chemical reaction is:

$2Cl_2(g)+7O_2(g)+130kcal\rightarrow 2Cl_2O_7(g)$

According to stoichiometry :

2 moles of $Cl_2O_7$ are produced by absorption of energy = 130 kcal

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Thus 780 kcal are required to produce 12.00 mol of $Cl_2O_7$

4 0

3 years ago

Strontium nitrate, Sr(NO3)2, is used in fireworks to produce brilliant red colors, Suppose we need to prepare 366.6 ml. of 0.115

natulia [17]

Answer:

$\boxed{\text{8.91 g}}$

Explanation:

1. Calculate the moles of Sr(NO₃)₂

$n = \text{366 mL} \times \dfrac{\text{0.115 mmol}}{\text{1 mL}}= \text{42.09 mmol}$

2. Calculate the mass of SrNO₃)₂

$m = \text{42.09 mmol} \times \dfrac{\text{211.63 mg}}{\text{1 mol}}= \text{8910 mg} = \text{8.91 g}\\\text{The mass of strontium nitrate required is }\boxed{\textbf{8.91 g}}$