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tigry1 [53]
3 years ago
13

Use the following Balanced Equation to complete the question: 2 Al + 6 HBr → 2 AlBr3 + 3 H2

Chemistry
1 answer:
leva [86]3 years ago
5 0
Here is the answer enjoy

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if 0.0203 g of a gas dissolves in 1.39 l of water at 1.02 atmospheres at what pressure (in atm) would you be able to dissolve 0.
Sergeu [11.5K]
First, we need to get n1 (no.of moles of water ): when

mass of water = 0.0203 g and the volume = 1.39 L

∴ n1 = mass / molar mass of water

        = 0.0203g / 18 g/mol
        = 0.00113 moles

then we need to get n2 (no of moles of water) after the mass has changed:

when the mass of water = 0.146 g

n2 = mass / molar mass

     = 0.146g / 18 g/ mol
     = 0.008 moles

so by using the ideal gas formula and when the volume is not changed:

So, P1/n1 = P2/n2 

when we have P1 = 1.02 atm 

and n1= 0.00113 moles

and n2 = 0.008 moles 

so we solve for P2 and get the pressure

∴P2 = P1*n2 / n1

        =1.02 atm *0.008 moles / 0.00113 moles

       = 7.22 atm

∴the new pressure will be 7.22 atm


5 0
3 years ago
Which elements, when they have to, can have more than
inn [45]
Elements in the third row can break the octet rule
6 0
3 years ago
What chemical bond will S and H form
Over [174]

Answer:

hydrogen sulfide (H2S)

Explanation:

8 0
3 years ago
What is the main purpose of using NaOH in the saponification reaction . NaOH works as the catalyst b. NaOH solution is the solve
Alex777 [14]

Answer:

C. NaOH acts as a reactant in the reaction

Explanation:

Because during the saponification process, Na+ replaces the H+ in the fatty acid been used for the saponification process

7 0
3 years ago
0.25 mol of nitric acid is used to make a 0.10 M nitric acid solution. How many grams of solute was used?
Yanka [14]

Answer:

15.75 grams of HNO3 was used and dissolved in 2.5 liters of solvent, to make a 0.10 M solution

Explanation:

Step 1: Data given

Nitric acid = HNO3

Molar mass of H = 1.01 g/mol

Molar mass of N = 14.0 g/mol

Molar mass O = 16.0 g/mol

Number of moles nitric acid (HNO3) = 0.25 moles

Molairty = 0.10 M

Step 2: Calculate molar mass of nitric acid

Molar mass HNO3 = Molar mass H + molar mass N + molar mass (3*O)

Molar mass HNO3 = 1.01 + 14.0 + 3*16.0

Molar mass HNO3 = 63.01 g/mol

Step 3: Calculate mass of solute use

Mass HNO3 = moles HNO3 * molar mass HNO3

Mass HNO3 = 0.25 moles * 63.01 g/mol

Mass HNO3 = 15.75 grams

15.75 grams of HNO3 was used and dissolved in 2.5 liters of solvent, to make a 0.10 M solution

7 0
3 years ago
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