All categories

2 years ago

What is the density of 96 ml of a liquid that has a mass of 90.5 g?

Chemistry

1 answer:

Otrada [13]2 years ago

8 0

Answer:

Density = Mass / Volume. so, x = 90.5 g / 96 mL ... The Density would be 0.942 g/mL

You might be interested in

If a solution at pH 5 undergoes a 1000-fold increase in [OH-], what is the resulting pH?

lara31 [8.8K]

<span>336*280 i believe... i hope this helps

</span>

7 0

2 years ago

2. After quenching your solution with ice, the resulting aqueous layer became acidic. Use a chemical equation to explain how the

alexandr402 [8]

Answer:

C2H5Cl + H20 ⇆ C2OOH4

Explanation:

The left over acetyl chloride which reacted with water to produce acetic acid

3 0

2 years ago

A system fitted with a piston expands when it absorbs 52.7J of heat from the surroundings. The piston is working against a press

Allushta [10]

Answer: The initial volume of the system is 60.29 L.

Explanation:

According to the first law of thermodynamics,

$\Delta U = Q - W$

As it is given that heat is being added to the system so, $\Delta H$ will be positive. And, work done on the system is negative and work done by the system is positive.

So here, $\Delta U$ = -107.4 J

Q = 52.7 J

P = 0.693 atm

And, W = PdV

or, W = $P (V_{final} - V_{initial})$

So, $\Delta U = Q - P (V_{final} - V_{initial})$

-107.4 J = 52.7 J - 0.693 \times 101.325 (63.2 - V)

-160.1 = -43.79 - 70.21 (63.2 - V)

63.2 - V = $\frac{160.1 + 43.79}{70.21}$

- V = 2.90 - 63.2

V = 60.29 L

Thus, we can conclude that the initial volume of the system is 60.29 L.

6 0

2 years ago

What mass (in grams) of aspirin (C₉H₈O₄) is produced from 57.6 g of C₇H₆O₃ assuming 95.0% yield from the reaction below? C₇H₆O₃

Vikentia [17]

Answer:

78.15 g

Explanation:

Number of moles of C₇H₆O₃ that reacted = mass/molar mass = 57.6g/126 gmol-1

Number of moles of C₇H₆O₃ = 0.457 moles of C₇H₆O₃

From the reaction equation;

1 mole of C₇H₆O₃ yields one mole of aspirin

0.457 moles of C₇H₆O₃ yields C₇H₆O₃ of aspirin

Hence theoretical yield of aspirin = 0.457 moles × 180 gmol-1 = 82.26g of aspirin

% yield = actual yield/theoretical yield ×100

Actual yield= % yield × theoretical yield/100

Actual yield = 95.0 × 82.26/100

Actual yield = 78.15 g

5 0

2 years ago

Suppose a solution is prepared by dissolving 15.0 g NaOH in 0.150 L of 0.250 M nitric acid. What is the final concentration of O

Kipish [7]

Answer:

2.25 M is the final concentration of hydroxide ions ions in the solution after the reaction has gone to completion.

Explanation:

Moles of NaOH = $\frac{15.0 g}{40 g/mol}=0.375 mol$

Molarity of the nitric acid solution = 0.250 M

Volume of the nitric solution = 0.150 L

Moles of nitric acid = n

$Molarity=\frac{Moles}{Volume(L)}$

$n=0.250 M\times 0.150 L=0.0375 mol$

$NaOH+HNO_3\rightarrow NaNO_3+H_2O$

According to reaction, 1 mole of nitric acid recats with 1 mole of NaOH, then 0.0375 moles of nitric acid will react with :

$\frac{1}{1}\times 0.0375 mol$ of NaOH

Moles of NaOH left unreacted in the solution =

= 0.375 mol - 0.0375 mol = 0.3375 mol

$NaOH(aq)\rightarrow Na^+(aq)+OH^-(aq)$

1 mole of sodium hydroxide gives 1 mol of sodium ions and 1 mole of hydroxide ions.

Then 0.3375 moles of NaOH will give :

$1\times 0.3375 moles=0.3375 mol$ of hydroxide ion

The molarity of hydroxide ion in solution ;

$=\frac{0.3375 mol}{0.150 L}=2.25 M$

2.25 M is the final concentration of hydroxide ions ions in the solution after the reaction has gone to completion.

3 0

2 years ago