Nitric acid can be produced from \[N{{H}_{3}}\] in three step process
I. \[4N{{H}_{3}}(g)+5{{O}_{2}}(g)\xrightarrow{{}}4NO(g)+6{{H}_{2}}O(g)\]
II. \[2NO(g)+{{O}_{2}}(g)\xrightarrow{{}}2N{{O}_{2}}(g)\]
III. \[3N{{O}_{2}}(g)+{{H}_{2}}O(l)\xrightarrow{{}}2HN{{O}_{3}}(aq)+NO(g)\]
% yield of Ist, IInd and IIIrd are respectively 40%, 50% and 70% respectively, then what volume of\[N{{H}_{3}}(g)\] sit 1 atm and \[0{}^\circ C\] required to produce 1075 g of \[HN{{O}_{3}}\]?
It is known that atoms have proton, neutron, electron and nucleus. If the mass of neutron assumed to be half of its original value whereas that of proton is assumed to be twice the original value, then the atomic mass of \[_{6}{{C}^{14}}\] will be
A 0.70 g sample consisting \[Ca{{C}_{2}}{{O}_{4}}\] and \[Mg{{C}_{2}}{{O}_{4}}\] is heated at \[300{}^\circ C,\] converting the two salts of \[CaC{{O}_{3}}\] and \[MgC{{O}_{3}}\]. The sample when weighs 0.47 g. If the sample had been heated to \[700{}^\circ C\] where the products are CaO and MgO. What would be the weight of mixture of oxides?
23.2 g of an organic compound having molecular formula \[{{C}_{n}}{{H}_{2n+2}}\] is burnt in excess of \[{{O}_{2}}(g)\]initially taken in a 44.82 L steel vessel. Before reaction the gaseous mixture w at 273 K with pressure of 2 aim. After complete combustion and loss of considerable amount of heat the mixture of product and excess of had a temperature of 546 K and 4.6 atm pressure. The formula of compound is
The volume of concentrated sulphuric acid which is 98% by mass (density \[=1.84\,g\,c{{m}^{-3}}\]) required to prepare \[5\,d{{m}^{3}}\] of \[0.5\text{ }mol\text{ }d{{m}^{-3}}\] solution of sulphuric acid is
Two elements X and Y have atomic weights of 14 and 16. They form a series of compounds A, B, C, D and E in which the same amount of element X, Y is present in the ratio 1 : 2 : 3 : 4 : 5. If the compound A has 28 parts by weight of X and 16 parts by weight of Y, then the compound of C will have 28 parts weight of X and
What weight of \[{{H}_{2}}{{C}_{2}}{{O}_{4}}\,\,2{{H}_{2}}O\,\,(\text{mol}\text{.}\,\text{wt}\text{.}\,=126)\] should be dissolved to prepare 250 ml of cent normal to be used as a reducing agent?
Apatite is a mineral that is found in tooth enamel. When fluoride toothpastes are used, this mineral is converted to fluoroapatite, which is more resistant to tooth decay. The formula of apatite is \[C{{a}_{5}}{{(P{{O}_{4}})}_{x}}F\]. What is the value of \[x\] if the compound contains 18.45% by weight of phosphorus? (Atomic weight of \[P=31,\,\,Ca=40,\]\[F=19\] and \[O=16\])
A silver coin weighing 11.34 g was dissolved in nitric acid. When sodium chloride was added to the solution all the silver (present as \[AgN{{O}_{3}}\]) was precipitated as silver chloride. The weight of the precipitated silver chloride was 14.35 g. Calculate the percentage of silver in the coin -
A self-contained breathing apparatus used \[K{{O}_{2}}\] to convert \[C{{O}_{2}}\] and \[{{H}_{2}}O\] in exhaled air into oxygen and \[KHC{{O}_{3}}\] as shown in the equation \[K{{O}_{2}}+{{H}_{2}}O+C{{O}_{2}}\xrightarrow{\,}\,KHC{{O}_{3}}+{{O}_{2}}\].
How many molecules of \[{{O}_{2(g)}}\] will be produced from the 0.044 g of \[C{{O}_{2(g)}}\] that is exhaled in a typical breath?
Three isotopes of an element have mass numbers M, (M + 1) and (M + 2). The mean atomic mass is (M + 0.5). Then which of the following ratio maybe accepted for M, (M + 1), (M + 2) respectively
A gaseous compound is composed of 85.7% by mass of carbon and 14.3% by mass of hydrogen. Its density is 22.8 g/L at 350 K and 1.0 atm pressure. Calculate the molecular formula of compound.
If 3 moles of \[{{H}_{2}}\] and 1 mole of \[{{N}_{2}}\] are completely converted into \[N{{H}_{3}},\] the ratio of initial and final volume at the same temp. and pressure will be:
1 mol of a gaseous aliphahatic compound\[{{C}_{n}}{{H}_{3n}}{{O}_{m}}\] is completely burnt in an excess of oxygen. The contraction in volume is (assume water get condensed out)
X and Y are two elements which form \[{{X}_{2}}{{Y}_{3}}\] and \[{{X}_{3}}{{Y}_{4}}\]. If 0.20 mol of \[{{X}_{2}}{{Y}_{2}},\] weighs 32.0 g and 0.4 mol of \[{{X}_{3}}{{Y}_{4}}\] weighs 92.8 g, the atomic weights of X and Y are respectively
Chlorophyll, the green colouring matter of plants responsible for photosynthesis, contains 2.68% of magnesium by mass. Calculate the number of magnesium atoms in 2.00g of chlorophyll.
Minimum amount of \[A{{g}_{2}}C{{O}_{3}}(s)\] required to produce sufficient oxygen for the complete combustion of C, H, which produces 11.2 ltr. of \[C{{O}_{2}}\] at S.T.P after combustion is: [Ag = 108] \[A{{g}_{2}}C{{O}_{3}}(s)\to 2Ag(s)+C{{O}_{2}}(g)+1/2{{O}_{2}}(g)\]\[{{C}_{2}}{{H}_{2}}+5/2{{O}_{2}}\to 2C{{O}_{2}}+{{H}_{2}}O\]
In the reaction \[4A+2B+3C\xrightarrow{{}}{{A}_{4}}{{B}_{2}}{{C}_{3}}\] what will be the number of moles of product formed. Starting from 2 moles of A, 1.2 moles of B & 1.44 moles of C:
About \[6\times {{10}^{-3}}\] mol \[{{K}_{2}}C{{r}_{2}}{{O}_{7}}\] reacts completely with \[9\times {{10}^{-3}}\] mol \[{{X}^{n+}}\] to give \[X{{O}^{-}}_{3}\] and \[C{{r}^{3+}}\]. The value of \[n\] is: