Question

A metal reacts with concentrated hydrochloric acid (12 M HCl) to give the soluble metal hexachloride based on the following reaction:

M (s) + 6 HCl (aq) → MCl6 (aq) + 3 H2 (g)

If it takes 23 mL of concentrated hydrochloric acid to fully dissolve 8.5 g of the metal, what is the identity of the metal?

Give the answer as the chemical symbol:

0.35 L of a P4 solution with a concentration of 0.70 M and 2.5 L of a Br2 solution with a concentration of 0.39 M react completely when mixed to give a single product. What is the product of the reaction?

A. PBr

B. PBr3

C. PBr5

D. P2Br4

E. P2Br8

A 5.00 g block of strontium metal (Sr) sits in 0.275 L of water.

Over time, oxygen gas (O2) in the water reacts with the metal to give strontium oxide. If the oxygen gas concentration in the water is 0.050 M, how many grams of the strontium metal will remain when all of the oxygen has reacted?

Answer #1

#

no. of mole = molarity X volume of solution in liter

23 ml = 0.023 liter

no. of mole HCl = 12 X 0.023 = 0.276 mole

According to reaction 6 mole of HCl react with 1 mole of metal M then to react with 0.276 mole of HCl requied mole of metal = 0.276 X 1 / 6 = 0.046 mole of metal

metal weight is 8.5 gm

thus 0.046 gm of metal = 8.5 gm then 1 mole of metal = 1 X 8.5 / 0.046 = 184.78 gm

molar mass of metal = 184.78 gm / mole

tungsten (W) have atomic weight = 183.84 gm is near about given calculated weight therefore identity of given metal is

**tungsten (W)**

Hydrochloric acid (HCl) reacts with sodium carbonate (Na2C3),
forming sodium chloride (NaCl), water (H2O), and carbon dioxide
(CO2). This equation is balanced as written:
2HCl(aq)+Na2CO3(aq)→2NaCl(aq)+H2O(l)+CO2(g)
Part A: What volume of 1.50 M HCl in liters is needed
to react completely (with nothing left over) with 0.250 L of 0.500
M Na2CO3?
Part B: A 621-mL sample of unknown HCl solution reacts
completely with Na2CO3 to form 15.1 g CO2. What was the
concentration of the HCl solution?
Please show work

Hydrochloric acid is usually purchased in a concentrated form
that is 37.0% HCl by mass and has a density of 1.20 g/mL. How much
concentrated solution would you take to prepare 2.75 L of 0.460 M
HCl by mixing with water?

0.727 g of an unknown metal is reacted with
excess concentrated hydrochloric acid according to the reaction
below. 0.335 L of hydrogen gas was
collected over water on a day when the temperature was
25.0 oC and the pressure was
0.98 atm. The vapor pressure of water at
25.0 oC is 23.8 torr.
Report the partial pressure of hydrogen gas in atmospheres, the
molar mass of the metal and the atomic symbol for the metal. The
ideal gas law constant R...

A 2.25 gram sample of zinc metal reacts with 5.00 grams of
hydrochloric acid to give zinc chloride and hydrogen gas according
the blanced equation:
Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) Molar mass ZnCl2: 136.28
g/mol
a. What is the limiting reactant?
b. What mass of ZnCl2 can be formed? (This is called the
theoretical yield.)

Aluminum metal reacts with hydrochloric acid to produce hydrogen
gas and aluminum chloride (write a balanced equation). When 1.357 g
of Al(s) is combined with 100.0 mL of 3.00M HCl (aq) in a coffee
cup calorimeter, all of the aluminum reacts, raising the
temperature of the solution from 21.5oC to 38.4oC. Find ΔHrxn in
kJ/mol H2. Assume the density of the solution is 1.00 g/mL and the
heat capacity is 4.184 J/goC. Attach a sheet of paper to show your...

A)
Zinc metal reacts with excess hydrochloric acid to
produce hydrogen gas according to the following
equation:
Zn(s) + 2HCl(aq) ------------>
ZnCl2(aq) + H2(g)
The product gas, H2, is collected over
water at a temperature of 20 °C and a pressure of
757 mm Hg. If the wet
H2 gas formed occupies a volume of
7.17L, the number of moles of Zn
reacted was ___________ mol. The vapor pressure of water is
17.5 mm Hg at 20 °C.
B) Oxygen...

Concentrated hydrochloric acid is 37.0% HCl by mass and has a
density of 1.18 g/mL. What is the molar concentration of
concentrated hydrochloric acid?

Zinc metal reacts with hydrochloric acid to produce zinc
chloride and hydrogen gas according to the equation below. What
volume of hydrogen gas would be produced at 0.998 atm and 27
degrees C if 15.11 g of zinc reacted with excess hydrochloric
acid?
Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g)

Zinc reacts with hydrochloric acid according to the reaction
equation
How many milliliters of 4.00 M HCl(aq) are required to react
with 7.95 g of Zn(s)?

According to a label on a bottle of concentrated hydrochloric
acid, the contents are 36.0% HCl by mass and have a density of 1.18
g/mL. What is the molarity of concentrated HCl. What volume of it
would you need to prepare 985 mL of 1.6 M HCl? What mass of sodium
bicarbonate would be needed to neutralize the spill if a bottle
containing 1.75 L of concentrated HCl dropped on a lab floor and
broke open?

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