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deff fn [24]
3 years ago
6

How many grams of hydrogen are needed to produce 1.80 g of water according to this equation? 2H2 + O2 → 2H2O

Chemistry
2 answers:
denpristay [2]3 years ago
8 0

Answer : The correct option is, (C) 0.200 g

Explanation : Given,

Mass of water = 1.80 g

Molar mass of water = 18 g/mole

Molar mass of H_2 = 2 g/mole

First we have to calculate the moles of water.

\text{Moles of }H_2O=\frac{\text{Mass of }H_2O}{\text{Molar mass of }H_2O}=\frac{1.80g}{18g/mole}=0.1mole

Now we have to calculate the moles of hydrogen gas.

The given balanced reaction is,

2H_2+O_2\rightarrow 2H_2O

From the balanced reaction we conclude that

As, 2 mole of water obtained from 2 mole of H_2 gas

So, 0.1 mole of water obtained from 0.1 mole of H_2 gas

Now we have to calculate the mass of hydrogen gas.

\text{Mass of }H_2=\text{Moles of }H_2\times \text{Molar mass of }H_2

\text{Mass of }H_2=(0.1mole)\times (2g/mole)=0.2g

Therefore, the mass of hydrogen gas required will be, 0.2 grams

s344n2d4d5 [400]3 years ago
4 0
Answer is c

Work out the moles of 2H2O: 1.80/ (16+1+1) = 0.1
The moles of 2H2 are the same (0.1)
The Mr of H2 is 2

So the mass needed to produce 1.80g of water is
0.1 x 2 = 0.2
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Jim wants to react hydrogen and oxygen to get 36 grams of water. If he starts with 4 grams of Hydrogen (H), then how many grams
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Answer:

Mass of Oxygen = 32 grams

Explanation:

Given:

Mass of water = 36 grams

Mass of Hydrogen = 4 grams

Find:

Mass of Oxygen

Computation:

Using Law of Conservation of mass

Mass of water = Mass of Hydrogen + Mass of Oxygen

36 grams = 4 grams + Mass of Oxygen

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3 0
3 years ago
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2 years ago
A sample of gas consists of 4.0 moles, and exists at stp. What is the volume of the gas?
faust18 [17]

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Explanation:

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6 0
2 years ago
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The goal of this lesson:
mote1985 [20]

Answer:

1. The concentration of N₂O₄ decrease as the temperature of the system increased.

2. The formation of products was favored by the addition of heat.

3. The reaction going from right to left is exothermic.

4. N₂O₄ → 2NO₂; HR = +14 kcal.

Explanation:

Equation of the reaction is as follows: N₂O₄ ⇄ 2NO₂

The forward reaction proceeds with an increase in temperature. As the temperature of the reaction was increased, more of the N₂O₄ decomposed to form NO₂. Therefore, the concentration of N₂O₄ deceased.

2. The formation of products, that is the forward reaction leading to formation of NO₂ was favored by the addition of heat. Thus, with increase in temperature, the concentration of NO₂ increased.

3. An endothermic reaction is a type of reaction which requires energy input in the form of heat in order to proceed.

From the observations during the reaction, an increase in temperature by the addition of heat resulted in an increase in the forward reaction, therefore, the forward reaction is endothermic and the backward reaction is exothermic. Thus, the reaction in which colorless N₂O₄ is produced, is an exothermic reaction.

4. The change in enthalpy of a reaction is the difference in the heat content of reactants and products. For exothermic reactions, enthalpy change is negative, whereas for endothermic reactions, enthalpy change is positive.

The decomposition of  N₂O₄ to NO₂ is an endothermic reaction. Hence, the correct chemical equation is: N₂O₄ → 2NO₂; HR = +14 kcal.

7 0
3 years ago
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V<span>an't Hoff factor (i) for NaCl solution is approximately 2.
</span>Van't Hoff factor (i) for glucose solution is 1.<span>
Change in freezing point from pure solvent to solution: ΔT = i · Kf · m.
Kf - molal freezing-point depression constant for water is 1,86°C/m.
m -  molality, moles of solute per kilogram of solvent.
</span>Kf and molality for this two solutions are the same, but Van't Hoff factor for sodium chloride is twice bigger, so freezing point is twice bigger.
8 0
3 years ago
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