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Natali [406]
3 years ago
13

Answer the following question: In a space shuttle, the CO2 that the crew exhales is removed from the air by a reaction within ca

nisters of lithium hydroxide. Let's assume that one astronaut exhales about 825. L of CO2 daily. What mass of water will be produced when this amount reacts with LiOH? The other product of the reaction is Li2CO3. When answering this question include the following:
Have both the unbalanced and balanced chemical equations.
Explain how to find the molar mass of the compounds.
Explain how the balanced chemical equation is used to find the ratio of moles (hint: step 3 in the video).
Explain how many significant figures your answer needs to have.
The numerical answer
Your Answer:
Chemistry
1 answer:
Ulleksa [173]3 years ago
6 0

Answer:

See Explanation

Explanation:

The unbalanced reaction equation is;

CO2(g) + LiOH(aq) + Li2CO3(aq) + H2O(l)

The balanced chemical reaction equation;

CO2(g) + 2LiOH(aq) + Li2CO3(aq) + H2O(l)

The molar mass of each compound is the sum of the relative atomic masses of the atoms of the elements that compose the compounds.

For CO2

12 + 16(2) = 12 + 32 = 44 g/mol

For LiOH

7 + 16 + 1 = 24 g/mol

For Li2CO3

2(7) + 12 + 3(16) = 74 g/mol

For H2O

2(1) + 16 = 18 g/mol

From the balanced chemical reaction equation, the mole ratio is 1:2:1:1. This is obtained from the stoichiometric coefficient of each reactant in the balanced chemical reaction equation.

From the question;

1 mole of CO2 occupies 22.4 L

x moles of CO2 occupies 825 L

x = 1 mole * 825 L/22.4 L

x = 36.8 moles

From the reaction equation;

1 mole of CO2 produces 1 mole of water

36.8 moles of CO2 produces 36.8 moles of water

Mass of 36.8 moles of water = 36.8 moles * 18 g/mol

= 662 g of water

The answer must have three significant figures because that is the same number of significant figures to which values were given in the question.

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Answer: The reaction is first order overall.

Explanation: Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

Rate=k[A]^x[B]^y

k= rate constant

For the given rate law:

Rate=k[A]^1[B]^1

x = 1= order with respect to A

y =1=  order with respect to B

n =( x+y)= (1+1) = 2 = Total order

a)  If [A] is doubled, the reaction rate will increase by a factor of 2: True

Rate'=k[2A]^1[B]^1

Rate'=k[2]^1[A]^1[B]^1

Rate'=[2]^1\times Rate

Rate'=[2]\times Rate

b) The reaction is first order overall: False

The overall order is 1+1= 2.

c)  k is the reaction rate constant: True

Rate=k[A]^x[B]^y

k= rate constant

d) The reaction is first order in [B]: True

For the given rate law:

Rate=k[A]^1[B]^1

x = 1= order with respect to A

e) The reaction is first order in [A]: True

For the given rate law:

Rate=k[A]^1[B]^1

y =1=  order with respect to B

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matrenka [14]

Adding heat to a system can encourage or increases a chemical reaction.

<h3>Change that can encourage a reaction</h3>

Increasing the temperature of a process, increase occurs in the average speed of the reactant molecules and we know that when more molecules move faster, the more number of molecules reacts with other molecules which results in faster formation of products.

In conclusion, adding heat is the right option.

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2 years ago
How many grams of N2 is needed to produce 2000 grams NH3?
BlackZzzverrR [31]

Answer:

1644 g

Explanation:

Step 1: Write the balanced equation

N₂ + 3 H₂ ⇒ 2 NH₃

Step 2: Calculate the moles corresponding to 2000 g of NH₃

The molar mass of NH₃ is 17.03 g/mol.

2000 g × 1 mol/17.03 g = 117.4 mol

Step 3: Calculate the moles of N₂ needed to produce 117.4 moles of NH₃

The molar ratio of N₂ to NH₃ is 1:2. The moles of N₂ needed are 1/2 × 117.4 mol = 58.70 mol

Step 4: Calculate the mass corresponding to 58.70 moles of N₂

The molar mass of N₂ is 28.01 g/mol.

58.70 mol × 28.01 g/mol = 1644 g

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