3CaCl2(aq) + 2Na3(PO4)(aq) - Ca3(PO4)2(s) + 6NaCl(aq) Molar Mass
Substance
g/mol
CaCl2
110.0
163.9
Na3(PO4)
Ca3(PO4)2
Naci
310.2
58.44
Use the balanced equation and the Molar Mass table above to answer the following question.
How much Ca3(PO4)2(s) could be produced in an industrial process if 55.00 g of CaCl2 in
solution reacted completely with sufficient Na3(PO4)(aq)?
А
310.2 g
B
155.1 g
103.4 g
D
51.70 g

20 drops hope this

10 years is the answer

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.