3 years ago

Which law relates to the ideal gas law? P 1 T 1 =P 2 T 2 P 1 n 1 =P 2 n 2 V 1 Omega 1 = V 2 n 2 P 1 V 1 = P 2 V 2

Chemistry

1 answer:

Kay [80]3 years ago

7 0

Answer:

Could you post another better looking question because I cannot understand this.

Explanation:

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13??? pls also explain how u do it

Lady_Fox [76]

Answer:

d. it has a high boiling point

Explanation:

all ionic compounds with ionic bonds have high boiling points

7 0

3 years ago

A sample of 28 Mg decays initially at a rate of 53500 disintegrations per minute, but the decay rate falls to 10980 disintegrati

prisoha [69]

Answer : The half life of 28-Mg in hours is, 6.94

Explanation :

First we have to calculate the rate constant.

Expression for rate law for first order kinetics is given by:

$k=\frac{2.303}{t}\log\frac{a}{a-x}$

where,

k = rate constant

t = time passed by the sample = 48.0 hr

a = initial amount of the reactant disintegrate = 53500

a - x = amount left after decay process disintegrate = 53500 - 10980 = 42520

Now put all the given values in above equation, we get

$k=\frac{2.303}{48.0}\log\frac{53500}{42520}$

$k=9.98\times 10^{-2}hr^{-1}$

Now we have to calculate the half-life.

$k=\frac{0.693}{t_{1/2}}$

$9.98\times 10^{-2}=\frac{0.693}{t_{1/2}}$

$t_{1/2}=6.94hr$

Therefore, the half life of 28-Mg in hours is, 6.94

8 0

3 years ago

When you decrease the volume of a gas, what happens to the temperature?

ale4655 [162]

the temperature is decreased

4 0

4 years ago

A 25 liter balloon holding 1.5 moles of carbon dioxide leaks. If we are able to determine that 0.9 moles of carbon dioxide escap

ad-work [718]

Answer:

10 Litre

Explanation:

Given that ::

v1 = 25L ; n1 = 1.5 mole ; v2 =? ; n2 = (1.5-0.9) = 0.6 mole

Using the relation :

(n2 * v1) / n1 = (n2 * v2) / n2

v2 = (n2 * v1) / n1

v2 = (0.6 mole * 25 Litre) / 1.5 mole

v2 = 15 / 1.5 litre

v2 = 10 Litre

3 0

3 years ago

What type of change is the process of solid ice changing into liquid water?

otez555 [7]

The change is called melting

6 0

3 years ago