Answer:
Average atomic mass = 51.9963 amu
Explanation:
Given data:
Abundance of Cr⁵⁰ with atomic mass= 4.34%
, 49.9460 amu
Abundance of Cr⁵² with atomic mass = 83.79%, 51.9405 amu
Abundance of Cr⁵³ with atomic mass =9.50%, 52.9407 amu
Abundance of Cr⁵⁴ with atomic mass = 2.37%, 53.9389 amu
Average atomic mass = 51.9963 amu
Solution:
Average atomic mass = (abundance of 1st isotope × its atomic mass) +(abundance of 2nd isotope × its atomic mass +....n) / 100
Average atomic mass = (4.34×49.9460)+(83.79×51.9405) +(9.50×52.9407)+ (2.37×53.9389) / 100
Average atomic mass = 216.7656 + 4352.0945 + 502.9367 +127.8352 / 100
Average atomic mass = 5199.632 / 100
Average atomic mass = 51.9963 amu
Answer:
4.90 moles of 
will produce (9.8) moles of 
,
(4.90) moles of 
and
(39.2) moles of 
Explanation:
From the question we are told that
The number of moles of is 
The formation reaction of is
From the reaction we see that
1 mole of is formed by 2 moles of 1 mole of and 4
This implies that
4.90 moles of will produce (2 * 4.90) moles of ,
(1 * 4.90) moles of and
(8 * 4.90) moles of
So
4.90 moles of will produce (9.8) moles of ,
(4.90) moles of and
(39.2) moles of
They have thier own group because because they have traits or metals and nonmetals
Answer:
C
Explanation:
Just look at the reactants.
2AgCl + BaBr2
The first reactant is made of 2 elements.
The second reactant is made of 2 elements.
It can't be a decomposition. At this level there is only one reactant made of 2 elements. Something like
2MgO ===> 2Mg + O2
is a decomposition. One compound breaking down into 2 elements Mg and O.
It can't be a combustion. One of the reactants in a combustion is oxygen. Those equations look like
C3H8 + 5O2 ==> 3CO2 + 4H2O
That would be what a combustion looks like
It can't be a single replacement. They look like
Mg + CuO ===> Cu + MgO
There are elements on both sides of the reaction.
that leaves a double replacement which I wrote about how you distinguish it.
Answer:
7L
Explanation:
Divide 101 by 10.1(kPa) and you get 10.
10 x .7 = 7
