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Bas_tet [7]
3 years ago
12

Ross (he was on break) pours water at 6.0 c into a container with a pressure of 23. torr. he then boils the water to a temperatu

re of 34
c. the volume changes to 18. ml and pressure to 78. torr. what was the initial volume of the water?
Chemistry
1 answer:
kodGreya [7K]3 years ago
8 0
For this question, since the parameters volume, pressure and temperature changes, we can use the combined gas law equation.
It states that PV/T = constant 
Therefore,
\frac{P1V1}{T1} =   \frac{P2V2}{T2}
Where parameters for the first instance are given on the left side and parameters for the second instance are given on the right side of the equation
Temperature in K - T1 = 6 °C + 273 = 279 K
                               T2 = 34 °C + 273 = 307 K
substituting the values in the equation
\frac{23.0 torr*V}{279K} =  \frac{78 torr*18 mL }{307 K}
V = 55.5 mL
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Write a balanced equation for the double-replacement precipitation reaction described, using the smallest possible integer coeff
ahrayia [7]

Answer:

NH4Br + AgNO3 —> AgBr + NH4NO3

Explanation:

When ammonium bromide and silver(I) nitrate react, the following are obtained as shown below:

NH4Br(aq) + AgNO3(aq) —>

In solution, NH4Br(aq) and AgNO3(aq) will dissociate as follow:

NH4Br(aq) —> NH4+(aq) + Br-(aq)

AgNO3(aq) —> Ag+(aq) + NO3-(aq)

The double displacement reaction will occur as follow:

NH4+(aq) + Br-(aq) + Ag+(aq) + NO3-(aq) —> Ag+(aq) + Br-(aq) + NH4+(aq) + NO3-(aq)

NH4Br(aq) + AgNO3(aq) —> AgBr(s) + NH4NO3(aq)

6 0
3 years ago
For an aqueous solution of sodium chloride (NaCl) .Determine the molarity of 3.45L of a solution that contains 145g of sodium
worty [1.4K]
Molar mass NaCl = 58.44 g/mol

number of moles:

mass NaCl / molar mass

145 / 58.44 => 2.4811 moles of NaCl

Volume = 3.45 L

Therefore :

M = moles / volume in liters:

M = 2.4811 / 3.45

M = 0.719 mol/L⁻¹

hope this helps!
6 0
3 years ago
Which element or elements are unbalanced in this equation?
Stells [14]

Answer:

Only the H is unbalanced.

Explanation:

There are 4 H's and 2 of everything else

7 0
3 years ago
Read 2 more answers
Please I need help on these 3 questions. Thank You.​
Liula [17]

1.

V = 200 mL (volume)

c = 3 M = 3 mol/L (concentration)

First we convert mL to L:

200 mL = 0.2 L

Then we calculate the moles using the formula: n = V × c = 0.2 L × 3 mol = 0.6 mol

Finally, we just use the molar mass of CaF2 to calculate the actual mass:

molar mass = 78 g/mol

The formula is: m = n × mm (mass = moles × molar mass)

m = 0.6 mol × 78 g/mol = 46.8 g

2.

For this question the steps are exactly like the first question.

V = 50mL = 0.05 L

c = 12 M = 12 mol/L

n = V × c = 0.05 L × 12 mol/L = 0.6 mol

molar mass (HCl) = 36.5 g/mol

m = n × mm = 0.6 mol × 36.5 g/mol = 21.9 g.

3.

The steps for this question are the opposite way.

m(K2CO3) = 250 g

molar mass = 138 g/mol

n = m ÷ mm = 1.81 mol

c = 2 mol/L

V = n ÷ c = 1.81 mol ÷ 2 mol/L = 0.905 L = 905 mL

6 0
3 years ago
What will be the volume of a gas sample at 358 K if its volume at 255 K is 7.4 L?
Jobisdone [24]

Answer:

10.4 L

Explanation:

V1/T1=V2/T2

V2= (V1*T2)/T1

V2= (7.4L * 358K)/255K

V2=10.4 L

4 0
3 years ago
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