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will anyone tell me about the tips of paper 5 n dependent ,independent variable
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Ya............independent variable is da one u r changing n dependent variable is a 1 that is supposed 2 b kept constant!will anyone tell me about the tips of paper 5 n dependent ,independent variable
these quations are given in data booklet so no need to memorize itA solution of Sn2+ ions will reduce an acidified solution of MnO4– ions to Mn2+ ions. The Sn2+ ions are oxidised to Sn4+ ions in this reaction.
How many moles of Mn2+ ions are formed when a solution containing 9.5 g of SnCl 2 (Mr: 190) is added to an excess of acidified KMnO4 solution?
help plzzzzzz
actually u might know water is amphoteric oxide and sulfuric acid is an acid this settles it i think u might be confused with 331 Which statements are correct in terms of the Brønsted-Lowry theory of acids and bases?
1 Water can act as either an acid or a base.
2 Sulfuric acid, H2SO4, does not behave as an acid when dissolved in ethanol, C2H5OH.
3 The ammonium ion acts as a base when dissolved in liquid ammonia.
Answer is 1 only, why?
31 Which statements are correct in terms of the Brønsted-Lowry theory of acids and bases?
1 Water can act as either an acid or a base.
2 Sulfuric acid, H2SO4, does not behave as an acid when dissolved in ethanol, C2H5OH.
3 The ammonium ion acts as a base when dissolved in liquid ammonia.
Answer is 1 only, why?
these quations are given in data booklet so no need to memorize it
Sn2+⇌ Sn4++ 2e- equation 1
(MnO4–)+ (8H+)+ 5e– ⇌ (Mn2+)+ 4H2O) equation 2
balance the number of electrons so that each equation have same number of electrons
multiply equation 1 by 5 and equation 2 by 5
and then add these equations we get
(16H+)+(5Sn2+)+2MnO4- yields (5sn4+)+2Mn2+
ignore the liquid we are concerned with ions and ions only
2moles of mno4- reacts with 5moles of sn2+
2/5moles of mn 1 moles sn
(9.5/190)*2/5 9.5/190
The table describes some of the chemistry and thermodynamic properties of the halogens.
Process ............... ..Name and Symbol of quantity2HX(g) → H2(g) + X2(g)...... enthalpy change of reaction, Hr
H2(g) + X2(g) *-->< 2HX(g).... equilibrium constant, Kp
X(g) → X+(g) + e–.................... ionisation energy, Hi
P.S * -->< means equilibrium reaction
Which statements about the relative values of these quantities are correct?
1 Hr for HCl > for HBr
2 Kp for HBr > Kp for HI
3 Hi for I > Cl
The answers are 1 and 2. But why ?
Can someone explain this ?
Thanks in advance.
1) Bond energy of HCl is higher than HBr, hence will has a high enthalpy change for HCl compare to HBr.
2) HBr bond energy higher tha HI, as if HBr formed, harder to form back to H2 and Br2, but it is easier for HI to form back H2 and I2, hence the Kp for HBr is higher than HI.
3) it is wrong as I is below Cl in Group 7, should have lower first ionisation energy
Hope this helps
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