From ca8d040ca14cb2ac01033fdeade3b38eca27a6b7 Mon Sep 17 00:00:00 2001 From: Dane Sabo Date: Tue, 3 Sep 2024 14:28:25 -0400 Subject: [PATCH] vault backup: 2024-09-03 14:28:25 --- .../2024-09-03 Homework 1.md | 2 +- 1 file changed, 1 insertion(+), 1 deletion(-) diff --git a/300s School/302. NUCE 2100 - Fundamentals of Nuclear Engineering/2024-09-03 Homework 1.md b/300s School/302. NUCE 2100 - Fundamentals of Nuclear Engineering/2024-09-03 Homework 1.md index bf8684fca..18d720729 100644 --- a/300s School/302. NUCE 2100 - Fundamentals of Nuclear Engineering/2024-09-03 Homework 1.md +++ b/300s School/302. NUCE 2100 - Fundamentals of Nuclear Engineering/2024-09-03 Homework 1.md @@ -34,7 +34,7 @@ $10 \text{g} \times \frac{1 \text{ mol } ^{12}\text{C}}{12 \text{g}} \times \fra *b. How many hydrogen atoms?* $2.77542 \text{ moles of water } \times \frac{2 \text{mol} H}{1 \text{mol} H_2O} \times \frac{0.6022045 \times 10^{24} \text{ atoms}}{1 \text{ mol }H} = 3.34274 \times 10^{24} \text{ H atoms}$ *c. How many deuterium atoms?* - $2.77542 \text{ moles of water } \times \frac{2 \text{mol} H}{1 \text{mol} H_2O} \times \frac{0.6022045 \times 10^{24} \text{ atoms}}{1 \text{ mol }H} = 3.34274 \times 10^{24} \text{ H atoms}$ + $3.34274 \times 10^{24} \text{ H atoms} \times \frac{0.0156 ^2H}{1 H} = 5.21468 \times 10^{22} \text{ deuterium atoms}$ **5. Find the mass of an atom of $^{235}\text{U}$** *a. in amu;* *b. in grams.*