WHAT IS THE PERCENT BY VOLUME OF ETHANOL IN A SOLUTION THAT CONTAINS 35 mL ETHANOL IN 115 mL OF WATER?

1 answer:

3 0

We need to first add both of the solution volumes together 35+115=150. Now we can divide the volume of the ethanol by the total volume 35/150=.233. To double check we can multiply the total volume by the percentage of ethanol by volume we got as a solution 150x.233=35. So the percentage by volume of ethanol in the solution is .233x100=23.3%.

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Calculate the amount of energy when water at 72 degrees c freezes completely at 0 degrees c

gtnhenbr [62]

Answer:

The amount of energy needed when water at 72 degrees c freezes completely at 0 degrees c is $6.37\times10^4$ Joules

Explanation:

$Q = m \times c \times \Delta T$

where

$\Delta T$ = Final T - Initial T

$Q_{1}=100 g \times 4.184 \frac{J}{g^{\circ} \mathrm{C}} \times\left(72^{\circ} \mathrm{C}-0^{\circ} \mathrm{C}\right)$

$Q_1$ =30125J

Q is the heat energy in Joules

c is the specific heat capacity (for water 1.0 cal/(g℃)) or 4.184 J/(g℃)

m is the mass of water

mass of water is assumed as 100 g (since not mentioned)

$Q_2$ is the heat energy required for the phase change

$Q_2$ =mass × heat of fusion

$\\$Q_{2}=100 g \times 336 \frac{J}{g}$\\\\$Q_{2}=33600 J$$

Total heat = $Q_1 + Q_2$

Total Heat = 30123J + 33600J

= 63725 J

= $6.37\times10^4$ Joules is the answer

3 0

3 years ago

A chemist found that 4.69 g of sulfur combined with fluorine to produce 15.81 g of a gas. what is the empirical formula of the g

timofeeve [1]

Mass of sulfur combined - 4.69 g
Mass of gas produced is 15.81 g, therefore mass of fluorine is (15.81-4.69) = 11.12 g
Number of sulfur moles - 4.69 g/32 g/mol = 0.15 mol
Number of fluorine moles - 11.12 g/ 19 g/mol = 0.585 mol
divide both by least number of moles
S - 0.15/0.15 = 1
F - 0.585/0.15 = 3.9 rounded off is 4
ratio of S to F = 1:4Therefore formula of the gas is SF₄

7 0

3 years ago

Read 2 more answers

how much heat energy is needed to raise the temperature of 78.4g of aluminum from 19.4 degrees c to 98.6 degrees c.

Iteru [2.4K]

The heat that is needed to raise the temperature of 78.4 g of aluminium from 19.4 °c to 98.6°c is 5600.77 j

calculation

Heat(Q) = mass(M) x specific heat capacity (C) x change in temperature(ΔT)

where;

Q=?

M = 78. 4 g

C=0.902 j/g/c