answer D
Explanation:hope thhis helped
Moles of ca3(po4)2 = 23.7 / 310.17 = 0.076
moles of (PO4)3- = 0.076 x 2 = 0.152
now, no. of ions = 0.152 x 6.022 x 10^{23}
= 9.2 x 10^{22}
The partial pressure of nitrogen in the problem is 725 - 231 = 494 mmHg.
494 / 760 = 0.650 atm. To continue, we will use the ideal gas equation to find the mole of N2 and from that, we can find the mass of N2.
PV = nRT ----> n= PV/RT
Find the mole of Nitrogen
Given P=0.650 atm
n= (0.650)x(255/1000) / (0.082 x 338)
= (0.650) (0.255) / 27.716
= 0.16575 / 27.716
= 0.0060 moles
Find the mass of nitrogen
G= n x Mr (N2)
= 0.0060 x 28
= 0.168 grams
So the mass of nitrogen is 0.168
<span>2H2 + O2 mc015-1.jpg 2H2O
</span><span>26.70 moles</span>
