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bezimeni [28]
3 years ago
5

The molar mass of water (H2O) is 18.0 g/mol. A sample of water has a mass of 18.0 g. How many moles of water are contained in th

is sample?
Chemistry
1 answer:
Ludmilka [50]3 years ago
3 0

The sample contains 1.00 mol H₂O.

Moles of water = 18.0 g H₂O × 1 mol H₂O/18.0 g H₂O = 1.00 mol H₂O

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True or false: If the pressure is constant, as the temperature of a gas increases the volume increases.
DerKrebs [107]

Answer:

False.

Explanation:

Because if there is more space in the container for the gas to move, there is less pressure.  There would be a decrease in the pressure

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3 years ago
Balance each of the following redox reactions occurring in basic solution.MnO−4(aq)+Br−(aq)→MnO2(s)+BrO−3(aq)Express your answer
Ahat [919]

Answer : The balanced chemical equation is,

2MnO_4^-(aq)+Br^-(aq)+H_2O(l)\rightarrow 2MnO_2(s)+BrO_3^-(aq)+2OH^-(aq)

Explanation :

Rules for the balanced chemical equation in basic solution are :

  • First we have to write into the two half-reactions.
  • Now balance the main atoms in the reaction.
  • Now balance the hydrogen and oxygen atoms on both the sides of the reaction.
  • If the oxygen atoms are not balanced on both the sides then adding water molecules at that side where the more number of oxygen are present.
  • If the hydrogen atoms are not balanced on both the sides then adding hydroxide ion (OH^-) at that side where the less number of hydrogen are present.
  • Now balance the charge.

The half reactions in the basic solution are :

Reduction : MnO_4^-(aq)+2H_2O(l)+3e^-\rightarrow MnO_2(s)+4OH^-(aq) ......(1)

Oxidation : Br^-(aq)+6OH^-(aq)\rightarrow BrO_3^-(aq)+3H_2O(l)+6e^-  .......(2)

Now multiply the equation (1) by 2 and then added both equation, we get the balanced redox reaction.

The balanced chemical equation in a basic solution will be,

2MnO_4^-(aq)+Br^-(aq)+H_2O(l)\rightarrow 2MnO_2(s)+BrO_3^-(aq)+2OH^-(aq)

8 0
3 years ago
Type the correct answer in the box. Express your answer to three significant figures. A balloon is filled with 0.250 mole of air
katrin2010 [14]

Answer:

∴ The absolute pressure of the air in the balloon in kPa = 102.69 kPa.

Explanation:

  • We can solve this problem using the general gas law:

<em>PV = nRT</em>, where,

P is the pressure of the gas <em>(atm)</em>,

V is the volume of the gas in L <em>(V of air = 6.23 L)</em>,

n is the no. of moles of gas <em>(n of air = 0.25 mole)</em>,

R is the general gas constant <em>(R = 0.082 L.atm/mol.K)</em>,

T is the temperature of gas in K <em>(T = 35 °C + 273 = 308 K</em>).

∴ P = nRT / V = (0.25 mole)(0.082 L.atm/mol.K)(308 K) / (6.23 L) = 1.0135 atm.

  • <em>Now, we should convert the pressure from (atm) to (kPa).</em>

1.0 atm → 101.325 kPa,

1.0135 atm → ??? kPa.

∴ The absolute pressure of the air in the balloon in kPa = (101.325 kPa)(1.0135 atm) / (1.0 atm) = 102.69 kPa.

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3 years ago
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Explain why the open ocean is often called a “marine desert”
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Blue Open

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