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MissTica
2 years ago
13

Propylene gas is used as a fuel. Consider the reaction of propylene gas (C3H6) with oxygen gas (O2). This combustion reaction pr

oduces carbon dioxide gas (CO2) and water vapor (H2O). Answer the questions below – in each case, assume the volume measurements occur at the same temperature and pressure.
Write a balanced equation for this reaction.

How many liters of oxygen gas is needed to burn 0.610 L of propylene gas completely? How do you know?

How many liters of carbon dioxide gas will be produced? How do you know?
Chemistry
1 answer:
blsea [12.9K]2 years ago
3 0

Answer:

C3H6 + 9/2 O2 ⇒ 3CO2 + 3 H2

according to the equation, mole of O2 =9/2 * mole of C3H6

so the liters of O2 gas = 9/2 * C3H6 gas = 9/2 * 0.61 =2.745l

similarly, according to the equation, CO2 gas = 3 * C3H6 gas=3*0.61=1.83l

Explanation:

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The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid

Explanation:

answer is correct

7 0
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In which situation are unbalanced forces acting on an object?(1 point)
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Answer:

1. Two people stand on the same side of a large tire. Both people pull the tire with equal force.

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5. The force acting on the object must be unbalanced.

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3 years ago
Whats the answer to #11
morpeh [17]

Well, one mole would be considered as 6.02 x 1023 (atoms). Which in the copper form, this would be considered to be as 63.66 grams of copper. Know, by knowing this information, we're now able to figured out the question.

53.3 ÷ (atoms) 6.02 x 1023 ...

Which as a result, we then have 2665 over.

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3 years ago
What is the healthy percentage of body fat for men?
Jet001 [13]

Answer:

Ideal body fat percentage for men

Category Percentage

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5 0
3 years ago
Calculate ΔG∘rxn for the following reaction:4CO(g)+2NO2(g)→4CO2(g)+N2(g).Use the following reactions and given ΔG∘rxn values:A)
mihalych1998 [28]

Answer : The   value of \Delta G^o_{rxn} for the reaction is -1131.4 kJ

Explanation :

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

The given main reaction is,

4CO(g)+2NO_2(g)\rightarrow 4CO_2(g)+N_2(g)    \Delta G^o_{rxn}=?

The intermediate balanced chemical reaction will be,

(1) 2NO(g)+O_2(g)\rightarrow 2NO_2(g)     \Delta G^o_1=-72.6kJ

(2) 2CO(g)+O_2(g)\rightarrow 2CO_2(g)     \Delta G^o_2=-514.4kJ

(3) \frac{1}{2}O_2(g)+\frac{1}{2}N_2(g)\rightarrow NO(g)     \Delta G^o_3=87.6kJ

Now we will reverse the reaction 1, multiply the reaction 2 by 2, reverse and half the reaction 3 and then adding all the equations, we get :

(1) 2NO_2(g)\rightarrow 2NO(g)+O_2(g)     \Delta G^o_1=72.6kJ

(2) 4CO(g)+2O_2(g)\rightarrow 4CO_2(g)     \Delta G^o_2=2\times (-514.4kJ)=-1028.8kJ

(3) 2NO(g)\rightarrow O_2(g)+N_2(g)     \Delta G^o_3=-2\times 87.6kJ=-175.2kJ

The expression for \Delta G^o_{rxn} will be,

\Delta G^o_{rxn}=\Delta G^o_{1}+\Delta G^o_{2}+\Delta G^o_{3}

\Delta G^o_{rxn}=(72.6kJ)+(-1028.8kJ)+(-175.2kJ)

\Delta G^o_{rxn}=-1131.4kJ

Therefore, the value of \Delta G^o_{rxn} for the reaction is -1131.4 kJ

3 0
3 years ago
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