A Sample Calculation: Prior to your first trial, try this sample calculation in

Question

A Sample Calculation: Prior to your first trial, try this sample calculation in order to estimate the mass of metal X needed in this experiment. a) Let's assume that you do this experiment and that you collect 30.0 mL of gas at a temperature of 23.0°C and an H2 pressure of 1.00 atm. Given this information, calculate the moles of hydrogen gas produced by the reaction. 0.03L T-25 K b) Given your answer in part a, how many moles of metal X reacted? Why? c) Now assume that X has a molar mass of 100 g/mol (the maximum possible). What Given your answer in part b, what was the initial mass of metal X? d) Now assume that X has a molar mass of 9 g/mol (beryllium, the minimum possible). What Given your answer in part b, what was the initial mass of metal X? 75

Explanation / Answer

Given that number of mole of H2 gas or answer of A is 0.0012338 moles

b)

assume that metal is bivalent than a common reaction is as follows:

X + 2HCl = MCl2 + H2

Here H2 = 0.0012338 moles

Now calculate the moles of Metal as follows:

0.0012338 moles         H2 * 1 mole metal X/ 1 mole H2

0.0012338 moles X

c)

given that molar mass of X = 100 g/ mole

amount of X = number of moles* molar mass

= 0.0012338 moles X *100 g/ mole

= 0.12338 g X

d)

Be2 + 4 HCl = 2 BeCl2 + 2 H2

given that molar mass of Be = 9 g/ mole

amount of Be number of moles* molar mass

= 0.0012338 moles Be *9 g/ mole

= 0.0.0111042 g Be

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.