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exis [7]
2 years ago
12

PLEASE

Chemistry
1 answer:
sesenic [268]2 years ago
7 0

Answer:

How many grams of H2 can be produced from the reaction of 11.5 grams of sodium with an excess of water? Hint: 2Na + 2H2O ---> 2NaOH + H2. Ans: 0.505g .

Explanation:

You might be interested in
What is the molarity of a solution that contains 0.220 moles KOH in 0.350 L of solution?
Lera25 [3.4K]

Answer:

0.628 M.

Explanation:

In order to solve this problem we need to keep in mind the<em> definition of molarity</em>:

  • Molarity = moles / liters

We are given both the <em>number of moles and the volume of solution</em>, meaning we can now proceed to <u>calculate the molarity</u>:

  • Molarity = 0.220 mol / 0.350 L
  • Molarity = 0.628 M
5 0
3 years ago
1.
Leya [2.2K]

Answer:

V₂ = 530.5 mL

Explanation:

Given data:

Initial temperature = 20.0°C

Final temperature = 40.0 °C

Final volume = 585 mL

Initial volume = ?

Solution:

Initial temperature = 20.0°C (20+273 = 293 K)

Final temperature = 40.0 °C (40+273 = 323 K)

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume  

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

V₁ = V₂T₁ /T₂  

V₂ = 585 mL × 293 K / 323 K

V₂ = 171405 mL.K / 323 K

V₂ = 530.5 mL

6 0
3 years ago
What volume would 3.01•1023 molecules of oxygen gas occupy at STP?
Sliva [168]
First, find moles of oxygen gas: (3.01 x10^23 molec.)/(6.02 x10^23) =0.5mol O2


Second, multiply moles by the standard molar volume of a gas at STP:(0.5mol)(22.4L) = 11.2L O2
6 0
3 years ago
What is the osmotic pressure of a solution made from 22.3 g of methanol (MM = 32.04 g/mol) that was added to water to make 321 m
xxMikexx [17]

Answer: The osmotic pressure of a solution is 53.05 atm

Explanation:

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

\pi=iMRT

Or,

\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT

where,

\pi = osmotic pressure of the solution = ?

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (methanol) = 22.3 g  

Volume of solution = 321 mL

R = Gas constant = 0.0821\text{ L.atm }mol^{-1}K^{-1}

T = temperature of the solution = 25^oC=[273+25]=298K

Putting values in above equation, we get:

\pi=1\times \frac{22.3\times 1000}{32.04\times 321}\times 0.0821\text{ L.atm }mol^{-1}K^{-1}\times 298K

\pi=53.05atm

Hence, the osmotic pressure of a solution is 53.05 atm

7 0
3 years ago
92dm3 of a gas dissolved in a solvent. How many moles is this?
Paul [167]
Assuming its at r. t.p and pressure
no. of moles = 96/24=4moles
altho some books will say that its 23.7dm3/mole but that doesnt really matter because its the process that matters
5 0
3 years ago
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