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kkurt [141]
3 years ago
15

P and Q are two substances such that the melting point of P and the boiling point of Q are the same. If P is a solid at a certai

n temperature, what state will Q be in at the same temperature?
Chemistry
1 answer:
Nimfa-mama [501]3 years ago
5 0

Answer:

Explanation:

Firstly, it should be noted that melting and freezing points are the same. Thus, when a substance melts at a certain temperature, it means it can also start freezing/solidifying at that same temperature. That been said, <u>when the substance P is a solid at a certain temperature, the other compound Q will boil at that same temperature and hence will be a gas at that same temperature</u>.

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The electron configuration belonging to the atom with the highest second ionization energy is ________.
Gemiola [76]

Answer:

Element Lithium

Explanation:

The element with the highest second ionization energy is lithium. It belongs to the alkaline metal group I.e group one metals

It has the highest second ionization energy because it is very difficult to remove the electron from the 1s orbital.

Its atomic number is 3. The electronic configuration is 1s2 2S1

5 0
3 years ago
How to answer this ?
nadezda [96]
You multiply (4×10)by*
6 0
3 years ago
1.  You have 10 grams of HCl, how many moles of HCl do you have?  
Oxana [17]

Explanation:

36.5gm (Molar mass) = 1mole

1 gram = 1/36.5 mole

10grams =(1/36.5) x 10 moles

= 0.027 x 10 moles

=0.27moles

4 0
2 years ago
If you have 222 g of radioisotope with a half-life of 5 days, how much isotope would remain after 15 days?
Dima020 [189]
If the half life is 5 days, you would have to divide 222 by 2 3 times.
so 222/2 =111g
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55.5/2 = 27.75g

after four half life the mass would be
27.75/2
13.875g

the percent would be
13.875/222
= 6.25%
7 0
3 years ago
In Part A, you found the amount of product (1.80 mol P2O5 ) formed from the given amount of phosphorus and excess oxygen. In Par
Finger [1]

First step is to balance the reaction equation. Hence we get P4 + 5 O2 => 2 P2O5

Second, we calculate the amounts we start with

P4: 112 g = 112 g/ 124 g/mol – 0.903 mol

O2: 112 g = 112 g / 32 g/mol = 3.5 mol

Lastly, we calculate the amount of P2O5 produced.

2.5 mol of O2 will react with 0.7 mol of P2O5 to produce 1.4 mol of P2O5.

This is 1.4 * (31*2 + 16*5) = 198.8 g

3 0
3 years ago
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