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lys-0071 [83]
2 years ago
13

A 3.5 L sample of gas at 25oC has an initial pressure of 86.7 kPa. The pressure of the gas decreases to 56.7 kPa as the gas expa

nds to volume of 8.00 L. What is the new temperature of the gas?
1. 445 K
2. 199 K
3. 310 K
4. 85.3 K
Chemistry
1 answer:
katrin2010 [14]2 years ago
8 0

Answer:

445K

Explanation:

according to universal gas theoreme, p1v1/T1=p2v2/T2

therefore, T2=(56.7×8×298)/(3.5×86.7)

≈445K

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3 years ago
Decreasing the temperature of the reaction 3H2 + N2<----->2NH3. In this reaction, the product absorbs heat. WHICH WAY WILL
AURORKA [14]

3H_{2}+N_{2}⇔2NH_{3}

Decreasing the temperature of the reaction,the reaction shifts forward.

The explanation is given below.

Explanation:

If the temperature of the reaction mixture is increased,then the equilibrium will shift to decrease the temperature.

If the temperature of the reaction mixture is decreased,then the equilibrium will shift to increase the temperature.

During the formation of the ammonia,it gives off heat.So it is an exothermic reaction.

3H_{2}+N_{2}⇔2NH_{3}

A decrease in the temperature favors the reaction that is exothermic (the forward reaction)because it produces energy.Therefore,if the temperature is decreased,the yield of the ammonia increases.

<em>Therefore if the temperature is increased,the reaction shifts forward and the yield of the ammonia increases and it is an exothermic reaction.</em>

7 0
3 years ago
If 10.0 mL of a .600 M of HNO3 reacts with 31.0 mL of .700M Ba(OH)2 solution, what is the molarity of Ba(OH)2 after the reaction
Tasya [4]

Answer:

<u></u>

  • <u>0.456M</u>

Explanation:

<u>1. Balanced molecular equation</u>

     2HNO_3+Ba(OH)_2\rightarrow Ba(NO_3)_2+2H_2O

<u>2. Mole ratio</u>

     \dfrac{2molHNO_3}{1molBa(OH)_2}

<u>3. Moles of HNO₃</u>

  • Number of moles = Molarity × Volume in liters
  • n = 0.600M × 0.0100 liter = 0.00600 mol HNO₃

<u>4. Moles Ba(OH)₂</u>

  • n = 0.700M × 0.0310 liter = 0.0217 mol

<u>5. Limiting reactant</u>

Actual ratio:

   \dfrac{0.0600molHNO_3}{0.0217molBa(OH)_2}\approx0.28

Since the ratio of the moles of HNO₃ available to the moles of Ba(OH)₂ available is less than the theoretical mole ratio, HNO₃ is the limiting reactant.

Thus, 0.006 moles of HNO₃ will react completely with 0.003 moles of Ba(OH)₂ and 0.0217 - 0.003 = 0.0187 moles will be left over.

<u>6. Final molarity of Ba(OH)₂</u>

  • Molarity = number of moles / volume in liters
  • Molarity = 0.0187 mol / (0.0100 + 0.0031) liter = 0.456M
5 0
3 years ago
For a tablet containing 500. mg of vitamin C, calculate how many ml of 0.095 M NaOH is required to reach the equivalence point.
Gala2k [10]

Answer:

mL of NaOH required =29.9mL

Explanation:

Let us calculate the moles of vitamin C in the tablet:

The molar mass of Vitamin C is 176.14 g/mole

moles=\frac{mass}{molarmass}=\frac{500mg}{176.14}=\frac{0.5}{176.14}=0.0028

Thus we need same number of moles of NaOH to reach the equivalence point.

For NaOH solution:

moles=MolarityXvolume=0.095Xvolume

0.00283=0.095Xvolume

volume=0.0299L=29.9mL

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