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krok68 [10]
3 years ago
13

Use the balanced equation given below to solve the problem that follows: Calculate the mass in grams of water produced along wit

h 5.0 L of CO2 at STP.
[ ] g H2O2

2 C2H2(g) + 5 O2(g --> 4 CO2(g) + 2 H2O(g)
**Your answer should be written as X.X
Chemistry
1 answer:
saveliy_v [14]3 years ago
6 0

Answer: 1.98 g

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given volume}}{\text{Molar volume}}  

\text{Moles of} CO_2=\frac{5.0L}{22.4L}=0.22moles

The balanced given equation is:

C_2H_2(g)+5O_2(g)\rightarrow 4CO_2(g)+2H_2O(g)  

According to stoichiometry :

4 moles of CO_2 will produce =  2 moles of H_2O

Thus 0.22 moles of CO_2 will produce=\frac{2}{4}\times 0.22=0.11moles  of H_2O

Mass of H_2O=moles\times {\text {Molar mass}}=0.11moles\times 18g/mol=1.98g

Thus 1.98 g of water is produced along with 5.0 L of CO_2 at STP

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Answer:

               The volume is increased.

Explanation:

                     According to <em>Charles' Law</em>, " <em>at constant pressure the volume and temperature of the gas are directly proportional to each other</em>". Mathematically this law is presented as;

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In statement the data given is,

T₁  =  10 °C  =  283.15 K                    ∴  K  =  273.15 + °C

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So, it is clear that the temperature is being increased hence, we will find an increase in volume. Let us assume that the starting volume is 100 L, so,

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Now, we will arrange equation 1 for V₂ as,

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Putting values,

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3 0
3 years ago
What is the molality of a solution of water and KCl if the freezing point of the solution is –3°C? (Kf = 1.86°C/m; molar mass of
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Some of the solutions exhibit colligative properties. These properties depend on the amount of solute dissolved in a solvent. These properties include freezing point depression, boiling point elevation, osmotic pressure and vapor pressure lowering. Calculations are as follows:

<span> ΔT(freezing point)  = (Kf)mi
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4 0
3 years ago
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dsp73

Answer:

5 moles of Fe

Explanation:

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