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Yuliya22 [10]
3 years ago
9

How many grams of nh3 can be produced from 3.80 mol of n2 and excess h2?

Chemistry
1 answer:
Sophie [7]3 years ago
4 0
The  balanced equation :N2 + 3H2 --> 2NH3

1) Let's find the molar mass of NH3 because it will be needed later.
 To determine the molar mass you have to consult the periodic table and see the atomic mass of each element. If the element is repeted, for example 3 times, you multiple the atomic mass per 3.
NH3= 14 + 1 x 3= 17 g/mol

2) By looking at the balanced equation, you can see that 2 mol of NH₃ were produced with only one mol of N2. How much NH3 will result when we have 3,80 mol of N2?
So now we solve it with a porportion:

2 mol NH3-------1 mol of N2
x               --------<span>3.80 of N2

x= 2 x3,8 = 7,6</span><span>mol NH3

3) </span> the only thing left to do is convert the moles obtained, to grams. We can use the formula:
nº of moles x molar mass= mass
7,6mol NH3  x 17 g/mol= mass of NH3
mass= 129,2 grams of NH3
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55 L of a gas at 25oC has its temperature increased to 35oC. What is its new volume?
ladessa [460]

Answer:

Approximately 56.8 liters.

Assumption: this gas is an ideal gas, and this change in temperature is an isobaric process.

Explanation:

Assume that the gas here acts like an ideal gas. Assume that this process is isobaric (in other words, pressure on the gas stays the same.) By Charles's Law, the volume of an ideal gas is proportional to its absolute temperature when its pressure is constant. In other words

\displaystyle V_2 = V_1\cdot \frac{T_2}{T_1},

where

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  • V_1 is the initial volume,
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Convert the temperatures to degrees Kelvins:

T_1 = \rm 25^{\circ}C = (25 + 273.15)\; K = 298.15\; K.

T_2 = \rm 35^{\circ}C = (35 + 273.15)\; K = 308.15\; K.

Apply Charles's Law to find the new volume of this gas:

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